At 25 ^oC,the highest osmotic pressure is ex | vedclass

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(A) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas

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$CaCl_2$

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(A) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.Since $C$,$R$,and $T$ are constant for all given solutions,the osmotic pressure depends directly on the van't Hoff factor $(i)$.For $CaCl_2$,$i = 3$ $(Ca^{2+} + 2Cl^-)$.For $KCl$,$i = 2$ $(K^+ + Cl^-)$.For Glucose and Urea,$i = 1$ because they are non-electrolytes.Since $CaCl_2$ has the highest value of $i$,it exhibits the highest osmotic pressure.

At $25 \ ^oC$,the highest osmotic pressure is exhibited by $0.1 \ M$ solution of

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